A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential |NO3(aq)+4H*(aq)+3e¯‍ - NO(g)+2H2O(l) = +0.96 V 'red 0 Ε red = +0.153 V 2+ Cu²+(aq)+e → Cu* (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. 中 Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? O О If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον No Yes ローロ e ☐ x10 G

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential |NO3(aq)+4H(aq)+3e¯‍ - NO(g)+2H2O(l) = +0.96 V 'red 0 Ε red = +0.153 V 2+ Cu²+(aq)+e → Cu (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. 中 Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? O О If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον No Yes ローロ e ☐ x10 G

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A certain half-reaction has a standard reduction potential E=+0.21 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? Data O yes, there is a minimum. E red = v If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. O no minimum Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is naximum. Pred = Iv If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum By using the information…
A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown: Co2+ (aq) + 2e → Co(s) Eº=-0.29 volt - Cd2+ (aq) +2e →→ Cd(s) E°= -0.42 volt The actual concentrations are: [Co2+ (aq)] = 0.0006 M, [Cd2+] = 0.149 M. What is the potential in volt of this galvanic cell? (T-298K) Report your answer with 3 places past the decimal point. Do not put unit in your answer.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e 2 Br (aq) = +1.065 V O,(9)+4H"(aq)+4e → 2H,0(1) E=+1.23 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the ローロ cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell Yes voltage under Explanation Check O2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Priv
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.753 M and [Ni2+]=0.0150 M. Use the standard reduction potentials in this table. Ni2+(aq) + 2e– → Ni(s)= -0.26 Zn2+(aq) + 2e– → Zn(s)= -0.76 Zn(s)+Ni2+(aq)↽−−⇀ Zn2+(aq)+Ni(s)
The electrochemical cell Cu|Cu 2+||Al 3+|Al has a potential of –1.997 V under standard conditions. What is the standard reduction potential for the reaction of Al 3+ Al?
A voltaic cell utilizes the following redox reaction and operates at 298 K: 3 Ce¹+ (aq) + Cr (s) → 3 Ce³+ (aq) + Cr³+ (aq) 1. What is the emf for this galvanic cell under standard conditions? 2. What is the emf of this cell when [Ce4+] = 3.0 M, [Ce³+] = 0.10 M, [Cr³+] = 0.010 M 3. What is the emf of this cell when [Ce4+] = 0.010 M, [Ce³+] = 2.0 M, [Cr³+] = 1.5 M
When [Cu²+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 2.806 V. What is the Mg2+ concentration in this cell? 2+ Cu²+ (aq) + Mg(s)→→ Cu(s) + Mg²+ (aq) [Mg2+1 = 8.11x10^-5 X mol/L
In the following: Al³+ (aq) + 3e → Al(s) E° = -1.66 V Cr³+ (aq) + 3e → Cr(s) E° = -0.74 V What is the standard cell potential for the corresponding galvanic cell? 0.00 V O-0.92 V +2.40 V +0.92 V O-2.40 V
Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Sn**] = 0.0666 M, [Fe*1 = 0.0301 M, [Sn*+] = 0.00345 M, and [Fe2+] = 0.01092 M. Standard reduction potentials can be found in this table. Sn²*(aq) + 2 Fe* (aq) = Sn*(aq) + 2 Fe²+*(aq) E = V
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu (aq) + 2A1 (s) 3Cu (s)+2A1* (aq) 2+ 3+ Suppose the cell is prepared with 2.15 M Cu“ in one half-cell and 7.31 M Al" in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. AL Rights
the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+ (aq) + Ba(s) → Sn (s) + Ba²+ (aq) 2+ 2+ in one half-cell and 3.14 M Ba Suppose the cell is prepared with 2.84 M Sn Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 ロ・ロ μ 00 09 Ś ? in the other.
Standard tables of reduction potentials assume standard conditions, but many electrochemical cells operate under nonstandard conditions. An electrochemical cell is constructed based on the following balanced equation: Cu(s) + 2 Ag*(aq) → Cu2+(aq) + 2 Ag(s) Half-reactions with standard reduction potentials are given below. Cu2+(aq) + 2 e¯ → Cu(s); E° = 0.342 V Ag*(aq) + e¯ → Ag(s); E° = 0.800 V 5th attempt See Periodic Table O Se Calculate Ecell at 298 Kfor an electrochemical cell based on the overall redox reaction between Cu2+ and Ag if [Ag*] = 2.56 × 10 Mand [Cu2+] = 8.25 x 10-4 M. 3 V